Transcript Hard-Soft Acid-Base Theory Definitions Arrhenius acids form hydronium ions in water, and bases form hydroxide ions.

Hard-Soft Acid-Base
Theory
Definitions
Arrhenius acids form hydronium ions in
water, and bases form hydroxide ions. This
definition assumes that water is the solvent.
Brønsted and Lowry expanded upon the
Arrhenius definitions, and defined acids as
proton donors and bases as proton acceptors.
They also introduced the concept of conjugate
acid-base pairs.
Other Solvents
For any solvent that can dissociate into a
cation and an anion, the cation is the acid, and
the anion is the base. Any solute that causes an
increase in the concentration of the cation is an
acid, those that increase the concentration of the
anion are bases.
Lewis Acids & Bases
The Lewis definition further expands the
definitions. A base is an electron-pair donor,
and an acid is an electron-pair acceptor. The
two combine to form an adduct.
A + :B  A-B
Lewis Acids & Bases
This definition includes the “standard”
Brønsted-Lowry acid-base reactions:
H+(aq) + :NH3(aq)  NH4+(aq)
It also includes the reactions of metal ions or
atoms with ligands to form coordination
compounds:
Ag+(aq) + 2 :NH3(aq)  Ag(NH3)2+(aq)
Lewis Acids & Bases
In addition, electron-deficient compounds
such as trivalent boron is categorized as a Lewis
acid.
B(CH3)3 + :NH3  (CH3)3B←NH3
The HOMO on the Lewis base interacts
with the electron pair in the LUMO of the
Lewis acid. The MOs of the adduct are lower in
energy.
Lewis Acids & Bases
The LUMO and
HOMO are called
frontier orbitals. If
there is a net lowering
of energy, the adduct
is stable.
BF3 + NH3
The LUMO of the acid, the HOMO of the
base and the adduct are shown below:
Lewis Acids & Bases
There is the possibility of competing
reaction pathways depending upon which
reactants are present, and the relative energies of
possible products. As a result, a compound
such as water may serve as an acid, a base, an
oxidizing agent (with Group IA and IIA metals)
or a reducing agent (with F2).
Lewis Acids & Bases
A Lewis base has an electron pair in its
highest occupied molecular orbital (HOMO) of
suitable symmetry to interact with the LUMO of
the Lewis acid. The closer the two orbitals are
in energy, the stronger the bond in the adduct.
Hard and Soft Acids and Bases
The polarizability of an acid or base
plays a role in its reactivity. Hard acids and
bases are small, compact, and nonpolarizable.
Soft acids and bases are larger, with a
more diffuse distribution of electrons.
Hard and Soft Acids and Bases
In addition to their intrinsic strength,
Hard acids react preferentially with hard bases, and soft
acids react preferentially with soft bases.
Examples: Aqueous Solubility
Silver Halides
Compound
AgF
AgCl
AgBr
AgI
solubility product
205
1.8 x 10-10
5.2 x 10-13
8.3 x 10-17
AgX(s) + H2O(l) ↔ Ag+(aq) + X-(aq)
Solubility of Lithium Halides
LiBr> LiCl> LiI> LiF
LiF should have a higher ∆solv than the other
salts, yet it is the least soluble in water. This is
due to the strong hard acid (Li+)/hard base (F-)
interaction.
Example: Thiocyanate Bonding
SCN- displays linkage isomerism as the ligand
coordinates to metals via the sulfur or the
nitrogen. Mercury (II) ion bonds to the sulfur (a
soft-soft interaction) whereas zinc ion bonds to
the nitrogen atom.
Example: K for ligand exchange
reactions
Compare:
[MeHg(H2O)]+ + HCl
MeHgCl + H3O+
K= 1.8 x 1012
[MeHg(H2O)]+ + HF
MeHgF + H3O+
K= 4.5 x 10-2
Hard and Soft Acids & Bases
There have been many attempts to
categorize various metal ions and anions to
predict reactivity, solubility, etc.
R.G. Pearson (1963) categorized acids and
bases as either hard or soft (using Kf values).
Hard acids bond in the order: F->Cl->Br->ISoft acids bond in the order: I- >Br- >Cl- > F-
Hard and Soft Acids & Bases
Hard acids or bases are compact, with the
electrons held fairly tightly by the nucleus. They
are not very polarizable. F- is a hard base, and
metal ions such as Li+, a hard acid.
Hard and Soft Acids & Bases
Large, highly polarizable ions are categorized
as “soft.” Iodide is a soft base, and transition
metals with low charge density, such as Ag+, are
considered to be soft acids.
Hard and Soft Acids & Bases
Hard acids tend to bind to hard bases.
Soft acids tend to bind to soft bases.
Problem

Predict the solubility (high or low) of silver
fluoride, silver iodide, lithium fluoride and
lithium iodide using the hard-soft acid/base
approach. Identify each Lewis acid and Lewis
base, and categorize each as hard or soft.
Charge Density – Hard Acids
Hard acids typically have a high charge
density. They are often metal ions with a
(higher) positive charge and small ionic size.
Their d orbitals are often unavailable to engage
in π bonding.
Charge Density – Soft Acids
Soft acids typically have lower charge density
(lower ionic charge and greater ionic size). Their
d orbitals are available for π bonding. Soft acids
are often 2nd and 3rd row transition metals with a
+1 or +2 charge, and filled or nearly filled d
orbitals.
Acids
Hard Acids
Borderline
H+, Li+, Na+, K+
Be2+, Mg2+, Ca2+
BF3, BCl3, B(OR)3
BBr3,B(CH3)3
Al3+,Al(CH3)3,AlCl3,AlH3
Cr3+,Mn2+, Fe3+, Co3+
Fe2+,Co2+,Ni2+
Cu2+,Zn2+,Rh3+
Ir3+, Ru3+, Os2+
SO3
SO2
Soft Acids
BH3,Tl+, Tl(CH3)3
Cu+,Ag+, Au+,
Cd2+,Hg22+,
Hg2+, Pd2+,Pt2+,
Pt4+
Acids – Effect of Oxid’n #
Hard Acids
Borderline
H+, Li+, Na+, K+
Be2+, Mg2+, Ca2+
BF3, BCl3, B(OR)3
BBr3,B(CH3)3
Al3+,Al(CH3)3,AlCl3,AlH3
Cr3+,Mn2+, Fe3+, Co3+
Fe2+,Co2+,Ni2+
Cu2+,Zn2+,Rh3+
Ir3+, Ru3+, Os2+
SO3
SO2
Soft Acids
BH3,Tl+, Tl(CH3)3
Cu+,Ag+, Au+,
Cd2+,Hg22+,
Hg2+, Pd2+,Pt2+,
Pt4+
Bases
Hard Bases
Borderline
F-, Cl-
Br-
Soft Bases
H-, I-
H2O, OH-,O2-
H2S, HS-, S2-
ROH, RO-, R2O, CH3CO2-
RSH, RS-, R2S
NO3-, ClO4CO32-,SO42-, PO43-
NH3, RNH2
NO2-, N3- , N2
SO32-
C6H5NH2, pyr
SCN-, CN-,RNC, CO
S2O32-
R3P, C6H6
Bases – effect of Oxid’n #
Hard Bases
Borderline
F-, Cl-
Br-
Soft Bases
H-, I-
H2O, OH-,O2-
H2S, HS-, S2-
ROH, RO-, R2O, CH3CO2-
RSH, RS-, R2S
NO3-, ClO4CO32-,SO42-, PO43-
NH3, RNH2
NO2-, N3- , N2
SO32-
C6H5NH2, pyr
SCN-, CN-,RNC, CO
S2O32-
R3P, C6H6
Effect of Linkage Site
SCN- vs. NCSThe nitrogen tends to coordinate with harder
acids such as Si, whereas the sulfur tends to
coordinate with softer acids such as Pt2+.
Effect of Oxidation Number
Cu2+/Cu+ on acid hardness
SO3/SO2 on acid hardness
NO3-/NO2- on base hardness
SO42-/SO32- on base hardness
Acid or Base Strength
It is important to realize that hard/soft
considerations have nothing to do with acid or
base strength. An acid or a base may be hard or
soft and also be either weak or strong.
In a competition reaction between two bases
for the same acid, you must consider both the
relative strength of the bases, and the hard/soft
nature of each base and the acid.
Acid or Base Strength
Consider the reaction between ZnO and
LiC4H9.
ZnO + 2 LiC4H9↔ Zn(C4H9)2 + Li2O
Zinc ion is a strong Lewis acid, and oxide
ion is a strong Lewis base.
Acid or Base Strength
Consider the reaction between ZnO and
LiC4H9.
ZnO + 2 LiC4H9↔ Zn(C4H9)2 + Li2O
soft -hard hard -soft
soft -soft
hard -hard
Zinc ion is a strong Lewis acid, and oxide
ion is a strong Lewis base. However, the
reaction proceeds to the right (K>1), because
hard/soft considerations override acid-base
strength considerations.
The Nature of the Adduct
Hard acid/hard base adducts tend to have
more ionic character in their bonding. These are
generally more favored energetically.
Soft acid/soft base adducts are more
covalent in nature.
Other Considerations

As the adduct forms, there is usually a change in
geometry around the Lewis acid site.
BX3 + N(CH3)3  X3B-NMe3
The stability of the adduct is:
BBr3 > BCl3> BF3
This order seems opposite of what would be
expected based on halogen size or
electronegativity.
Other Considerations
empty 2p orbital
The reactivity pattern
suggests some degree of
π bonding in BF3.
filled orbitals
Other Considerations

Steric factors can play a role. An example is the
unfavorable reaction between :N(C6H5)3 and
BCl3. The large phenyl groups interact with the
chlorine atoms on boron to destabilize the
product.
Applications of Hard/Soft Theory
The Qual Scheme, a series of chemical
reactions used to separate and identify the
presence of dozens of metal ions, is based
largely on the hard and soft properties of the
metal ions.
The softer metals are precipitated out as
chlorides or sulfides, with the harder ions
formed as carbonates.
Evidence in Nature
In geochemistry, the elements in the earth’s
crust are classified as lithophiles or chalcophiles.
The lithophile elements are typically found
as silicates (bonded via the O atom): Li+, Mg2+,
Ti3+, Al3+ and Cr2+,3+. These are hard Lewis
acids.
Evidence in Nature
The chalcophile elements are typically found
as sulfides or bonded to Se2- or Te2-. They
include: Cd2+, Pb2+, Sb3+, and Bi3+. These are
soft Lewis acids. Zinc ion, which is borderline,
is typically found as a sulfide.